1. The problem statement, all variables and given/known data How much ice (in grams) would have to melt to lower the temperature of 351 ml of water from 24 deg C to 5 deg C? (Assume the density of water is 1.0g/ml .) 2. Relevant equations q=mc(deltaT) 3. The attempt at a solution m=351 g c=4.18J/g*C deltaT=19deg C q=27.88kJ then heat of fusion = 6.02kJ/mol take 27.88/6.02 = 4.631 mol * 18.02g/mol= 83.45 grams. this is wrong. the only problem i see is where i used the specific heat of water instead of ice. spec heat of ice=2.09. should I use the spec heat of ice instead of water? thanks!